The equilibrium of the reaction CO + H2O = CO2 + H2 deltaH = 42kJ will shift to the left, if: a) the pressure increases b) the H2O concentration increases c) CO2 concentration decreases d) lower the temperature

1. 2NO(g) + O₂(g) ⇒ 2NO₂(g) Consider the reaction Which would decrease the partial pressure of NO₂(g) at equilibrium? A) Increasing the volume of the system B) Adding a noble gas to increase the pressure of the system C) Adding NO(g) to the system D) Adding an appropriate catalyst E) Decreasing the volume of the system for which ΔΗ<0.

The synthesis of CaCO3 uses this chemical reaction. CaO(aq) + CO2(g) ——> CaCO3(s) + 180 kJ Identify three stresses that can be imposed on the equilibrium to maximize the amount of CaCO3 present. Be specific about what, if any, compounds are involved in those stresses.

1. For the reaction: 2NH3(g) + CO2(g) (NH2)2CO(s) + H2O(g) AH = - 330 kJ Predict how each of the following changes would impact a reaction that is currently at equilibrium. That is, which way would the reaction progress in order to respond to the change in the system to regain equilibrium (use arrows to show the direction of change that would occur to return back to equilibrium). Explain your reasoning for each part.